The reaction of peroxydisulfate ion ( S,0g-) with iodide ion (1") isS,03 (ag) + 31 (aq) → 2s0, (ag) + I3 (ag)From the following data collected at a certain temperature, determine the rate law and calculate therate constant.Experiment [S20g²](M) (M)0.0400Initial Rate [M/s]6.80 x 103.40 x 1010.030020.03000.020030.06000.02006.80 x 104(a) Which of the following equations represents the rate law for this reaction?A. rate = k[S,Og]ŋB. rate = k[S,Og 0C. rate = k[S,Og?0D. rate = k[S,Og o²Аово сор(b) What is the rate constant for the reaction?k=M's

The sum of the exponent term in the rate law for a chemical reaction is known as the order of the…

The reaction of peroxydisulfate ion (S,05) with iodide ion (1) is s,0g (aq) + 31 (aq) → 2s0, (aq) + I3 (aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. [S;Os1(M) [](M)| 0.0300 Experiment Initial Rate [M/s] 6.80 × 10 3.40 x 10 6.80 × 10 1 0.0400 0.0300 0.0200 3 0.0600 0.0200 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S;OgO B. rate = k[S,Og7n C. rate = k[S,Og0 D. rate = k[S,0g o %3D Aово сор (b) What is the rate constant for the reaction? M's

The reaction of peroxydisulfate ion (S,05) with iodide ion (1) is s,0g (aq) + 31 (aq) → 2s0, (aq) + I3 (aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. [S;Os1(M) [](M)| 0.0300 Experiment Initial Rate [M/s] 6.80 × 10 3.40 x 10 6.80 × 10 1 0.0400 0.0300 0.0200 3 0.0600 0.0200 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S;OgO B. rate = k[S,Og7n C. rate = k[S,Og0 D. rate = k[S,0g o %3D Aово сор (b) What is the rate constant for the reaction? M's

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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7. The reaction between the peroxydisulfate ion (S,0,2-) and the iodide ion (I) is: S,0g +31, (aq) (aq) (aq) a. From the following data (Table below), which were collected at a set temperature, determine the rate law and calculate the specific rate constant. %3D [I] (М) Initial Rate b=8-riós Experiment (М) (M/s) 1 0.080 0.034 2.2 x 10 4 0.080 0.017 1.1 x 10-4 3. 0.16 0.017 2.2 x 104 b. What is the initial rate of reaction if the concentrations of both S2O82- and |- are 0.5 M?
The reaction between selenous acid and the iodide ion in acid solution is H2SEO3(aq) + 61 (aq) + 4H*(aq) Se(s) + 213 (aq) + 3H20() The data in the following table were measured at 0°C. Experiment [H2SeO3lo (M) [H*]o (M) ] (M) Initial Rate [mol/(L )] 1.00 x 10-4 2.00 x 10-2 3.00 x 10-2 5.30 x 10-7 2.00 x 10-4 2.00 x 10-2 3.00 x 10-2 1.06 x 10 6 3.00 x 10 4 4.00 x 10-2 3.00 x 10 2 6.36 x 10-6 4 3.00 x 10-4 8.00 x 10-2 3.00 x 10-2 2.54 x 10-5 3.00 x 10-4 8.00 x 10-2 6.00 × 10-2 2.04 x 10-4 2.00 x 10-4 2.00 x 10-2 Tripling the initial concentration of H,SeO, while holding the initial concentrations 6.00 x 10-2 8.48 x 10-6 of Ht and I constant increases the rate of the reaction by a factor of 8. 4. 3. 1. 23 2.
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The thermal decomposition of PH3 is a first order process: 4 PH3(g) → P4(g) + 6 H2(g) If the value for the rate constant, k equals 2.00 x 10-2/sec, how long (sec) would it takes for 85% of the PH3 to decompose? Express the answer to 3 sig. figs. ln[A]t = -kt + ln[A]o
The decomposition of nitramide, O₂NNH,, in water has the chemical equation and rate law [O₂NNH₂] [H+] O₂NNH, (aq)- -N₂O(g) + H₂O(1) A proposed mechanism for this reaction is 1.0,NNH, (aq) = O,NNH(aq) + H+ (aq) (fast equilibrium) rate = k 2.0, NNH (aq) N₂O(g) + OH- (aq) (slow) 3. H(aq) + OH-(aq) H₂O(l) (fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? k₂ Answer Bank k_ k3 k
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The reaction 21(aq) + S,Og²(aq) - »(aq) + 2SO,*(aq) was studied at 25°C. The following results were obtained where A[S,0, ] 2- Rate At [I] (mol/L) [S,Og*]o (mol/L) Initial Rate (mol/L • s) 12.5×10" 6.25×106 6.25×106 5.00×10-6 7.00×106 0.080 0.040 0.040 0.040 0.080 0.020 0.032 0.040 0.060 0.030 (a) Determine the rate law. (b) Determine the rate constant.
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y = mz +b. • Part A Order Integrated Rate Law Graph Slope [A] =- kt + [A]Jo -kt + In[A]o In[A] vs. t + = kt + TAT [A] vs. t -k The reactant concentration in a zero-order reaction was 7.00x102 M after 170 s and 3.00x102 M after 380 s. What is the rate constant for this reaction? 1 In[A] = -k Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. 1 - vs t JA 2 • View Available Hint(s) ? koih = Value Units Submit Prevlous Anawera Part B Complete previous part(s) • Part C The reactant concentration in a first-order reaction was 6.60x102 Mafter 30.0 s and 7.70x10 Mafter 100 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a…